Write the equilibrium-constant expressions and obtain numerical values for each constant ina. the basic dissociation of ethyl amine, C2H5NH2.b. the acidic dissociation of hydrogen cyanide, HCN.c. the acidic dissociation of pyridine hydrochloride, C5H5NHC1.d. the basic dissociation of NaCN.e. the dissociation of H3ASO4 to H³O* and AsO,-f. the reaction of CO;2- with H2O to give H2C03and OH-

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Answered: Write the equilibrium-constant…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.65PAE

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. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)
Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
Write the equilibrium-constant expressions and obtain numerical values for each constant in (c) the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. (d) the basic dissociation of NaNO2. (e) the dissociation of H3AsO3 to H3O+ and AsO33-
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calcul the concentration of H+ if the initial concentration of acid is 0.100 M. d Q4- How many grams of sodium hydroxide (M.wi=58.5) can be added 0 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changi POH by more than lunit? Ky=1.8x 10°? w
HF is a weak acid, whose conjugate base is F-. Write the reaction that corresponds to Ka and Kb for the respective species. Write the equilibrium expression for each reaction.
Write the acid dissociation constant expression for nitrous acid, HNO2.
Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
At equilibrium, the value of [H+] in a 0.260M solution of an unknown acid is 0.00405M . Determine the degree of ionization and the Ka of this acid.
At a certain temperature, a solution of ammonia at equilibrium is found to have concentrations of the weak base equal to 0.0497 M and of OH- and the conjugate acid equal to 1.01x10-3 M. What is the value of the base ionization constant, Kb, at this temperature?
Palmitic Acid, CH3(CH2)14COOH, found in both bacon fat and many soaps. Palmitic acid partially ionizes in water. Write a balanced chemical reaction for the dissociation of palmitic acid into its conjugate base and hydrogen ion. Write an expression for the equilibrium constant for palmitic acid. The equilibrium concentrations are [CH3(CH2)14COOH] = 0.1 M and [H+] = [CH3COO-] = 0.0133352 M. Calculate the equilibrium constant of ionization KA. Calculate the pKA of palmitic acid. Draw (by hand) the titration curve for palmitic acid. Please label your axes appropriately.

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Write the equilibrium-constant expressions and obtain numerical values for each constant in a. the basic dissociation of ethyl amine, C2H5NH2. b. the acidic dissociation of hydrogen cyanide, HCN. c. the acidic dissociation of pyridine hydrochloride, C5H5NHC1.